Rutherfords Model of Atoms and Its Limitations

Edited By Team Careers360 | Updated on Jul 02, 2025 04:39 PM IST

Rutherford Model of Atoms and its Limitation and its Limitation

A model of plum pudding provided by J. J. Thomson failed to explain certain experimental results associated with the formation of atomic material. Ernest Rutherford, a British scientist who conducted the study and based on the observations of the study, proposed the atomic composition of the elements and presented the Rutherford atomic model.

This Story also Contains

Rutherford Model of Atoms and its Limitation and its Limitation
Conclusion of Rutherford Alpha Scattering Experiment
Explain Rutherford model of an atom:
Limitations of Rutherford Atomic model:
According to Rutherford's atomic model:
Maxwell's Atomic Model

Rutherford's scattering test of Alpha

Rutherford experiment performed the experiment by blasting a small sheet of gold with α particles and then studying the traces of these particles after their contact with the gold wire. To study the deviations caused by α particles, he placed a fluorescent zinc sulphide screen around a small gold plate. Rutherford experiment made some observations that contradicted Thomson's atomic model.

Also read -

Conclusion of Rutherford Alpha Scattering Experiment

Rutherford alpha particle scattering experiments led him to the conclusion that:

A large portion of the α particles attacked by the gold leaf pass through it without deviation, which is why most of the atomic space is empty. In Rutherford scattering experiment some α particles were purified by a gold sheet at very small angles, which is why a positive charge atom can be transmitted equally. Good atomic charging is focused on very small volumes. There are very few α-retrospective particles, i.e. only a few particles with a 180o deviation angle. The volume at which particles are well deposited atoms is therefore relatively small compared to the total atomic mass.

Explain Rutherford model of an atom:

Based on the above observations and above conclusions, Rutherford proposed the formation of atomic elements.

According to Rutherford's atomic model:

The well-charged particles and the atomic mass were concentrated in an extremely small volume. He called this atomic region a nucleus. Rutherford's model suggested that electrons were negatively charged around the nucleus of an atom. He also said that the electrons around the nucleus rotate at very high speeds in circular paths. He named the circular paths as a trail. Electrons are poorly charged and the nucleus is a massive mass of well-charged particles held together by a powerful magnetic field.

Limitations of Rutherford Atomic model:

Rutherford suggested that electrons revolve around the nucleus in a fixed pattern called orbits. According to Maxwell, fast-moving particles emit electromagnetic radiation and that is why the electrons around the nucleus must emit electromagnetic radiation. This radiation will carry energy from the electron movement which will come at the expense of the reduction of the radiation.

Statistics have shown that according to Rutherford's model, the electron will fall to the nucleus in less than 10-8 seconds. Rutherford's model was therefore in conflict with Maxwell's theory and could not explain atomic stability. One of the drawbacks of Rutherford's model is that he did not say anything about the arrangement of electrons in atoms that made his theory incomplete. Although early atomic types were inaccurate and failed to explain certain experimental results, they were the basis for future developments in the world of quantum mechanics.

Also read :

NEET Highest Scoring Chapters & Topics

This ebook serves as a valuable study guide for NEET exams, specifically designed to assist students in light of recent changes and the removal of certain topics from the NEET exam.

Download EBook

What did Rutherford discover?

A complete experiment, Rutherford (1871-1937) was in charge of a remarkable series of discoveries in the field of radioactivity and nuclear physics.

It detects alpha and beta rays, sets the rules for radiation decay, and identifies alpha particles such as helium nuclei.

What did Rutherford Discover About the Atom?

Ernest Rutherford is known for his pioneering studies in radioactivity and atoms. He found that there are two types of radiation, alpha and beta, from uranium. You have found that most of the atoms have a blank space, and their size is cantered on the well-charged central part.

What did Rutherford find in his analysis of the gold plate?

Examination of the foil of gold has shown that the atom has a tiny, large, well-charged cell with poorly charged electrons at a distance from the centre. Niels Bohr built on Rutherford's model to make his own.

Related Topics Link,

How deep was the gold plate in Rutherford's Research?

Size 0,00004 cm

Gold plate of only 0.00004 cm members. Most of the alpha particles went directly to the disc, but some were distorted by the disc and hit the screen on one side. Geiger and Marsden found that about 1 in 20,000 alpha particles were deviated by 45 ° or more. The Main Postulates Of Rutherford atomic model

According to Rutherford's atomic model:

Rutherford's model suggested that electrons were negatively charged around the nucleus of an atom. The well-charged particles and the atomic mass were concentrated in an extremely small volume. He called this atomic region a nucleus. Rutherford also said that the electrons around the nucleus rotate at very high speeds on circular paths. He named the circular paths as a trail. Electrons are poorly charged and the nucleus is a massive mass of well-charged particles held together by a powerful magnetic field.

Reason for Failure of the Rutherford atomic model

The electron orbital is not expected to stabilize. Rutherford's model was unable to explain the stability of the atom. Rutherford's model did not explain the design of the electron atoms that made his theory incomplete. According to Rutherford's example, electrons would lose energy as they traveled in their orbit. This will allow them to slow down a bit and move on to the other side. The electron will follow the wind path and enter the nucleus. Eventually the atom would collapse. But in reality, the atom is stable.

What was the source of the alpha particles?

Alpha (α) particles are well charged and are composed of two protons and two neutrons from the nucleus of an atom. Alpha particles are derived from the decay of highly radioactive substances, such as uranium, radium and polonium.

How did Rutherford produce the alpha particles?

The new line was very simple, a chemical process mixed with physics. For this work Rutherford hired Thomas Royds (1884-1955), who had graduated with a degree in Physics Honors in 1906. They collect α particles in a closed glass tube, press them, and transmit an electric spark.

What is Electromagnetic Radiation?

Whenever money is invested in electricity or magnetic fields, it has a certain amount of energy to work, or in the case of many cases, they are reunited.

Maxwell's Atomic Model

In 1870, James Maxwell became the first scientist to describe the interdependence of existing electric-and-magnetic fields. He suggested that when electrical particles make rapid movements, magnetic fields are exchanged and transmitted. These camps travel through the types of waves known as electromagnetic waves. The light wave is an example of electric radiation.

NCERT Chemistry Notes:

Electromagnetic Radiation Features:

The charge-generating particles produce attractive electric and electric fields adjacent to each other and both point to the direction of wave propagation. Electric waves do not need a medium, that is, they can also travel in an empty space. There are many types of electromagnetic radiation, which differ from each other in terms of length of frequency or frequency. This total electromagnetic radiation together creates an electric spectrum. For example radio frequency region, microwave region, eye region, ultraviolet region, visual region etc. Electromagnetic radiation is characterized by various properties such as frequency, duration, duration, etc.

Electromagnetic Radiation Formula

Frequency is defined as the number of waves exceeding a given point in one second. Statistically it is equal to the frequency of electromagnetic radiation. A typical equation with the speed of light, frequency, and length of electromagnetic radiation is given below:

c = ν ?

Where,

c = light speed,

ν = frequency and frequency

? = wavelength.

In addition to the frequency and length of time, some other parameters are used to separate the electromagnetic rays. Mathematically, it is equal to the frequency of wavelengths. Shown in SI unit as m^-1.

Also check-

Frequently Asked Questions (FAQs)

1. 1.What is the magnitude of electromagnetic radiation?

Electromagnetic radiation (EM) is a source of energy that is distributed in the form of electric waves through free space or through a tangible object. The dual presence of electromagnetic radiation: reflects wave and particulate (photon) properties.

2. 2.What is the nature of the waves?

Long-term wave disturbance that travels like air or water through the center. Beverages like these can be thought of as having “particles” composed of a large number of individual molecules.

3. 3.Is radiation harmful to humans?

There is no doubt that exposure to very high levels of electromagnetic fields in the short term can be detrimental to health. Without thorough research, there is no reason to make a date to suggest that the exposure of low-level electric fields is contrary to human health.

4. 4.What are electric waves and their components?

EM waves climb into the hole with a fixed frequency of 3.00 x 10⁸ ms^-1. The electric field, or gravity, does not deviate. They can show disruption or spread, however. Electric shock - either air, solid object or vacuum - can go beyond anything.

5. 5.Is the electric field light?

Radiation by radio waves, gamma-ray, visible light, and all other electromagnetic spectrum objects. With regard to the diffusion of very small particles, called photons, each moving at the speed of light with a wave-like pattern, electric beams can be represented.

6. How does Rutherford's model differ from Thomson's "plum pudding" model?

Rutherford's model proposes a small, dense nucleus with electrons orbiting around it, while Thomson's model suggested that electrons were embedded uniformly throughout a positively charged sphere. Rutherford's model introduced the concept of a nucleus and mostly empty space within the atom.

7. What is the significance of "mostly empty space" in Rutherford's atomic model?

The concept of atoms being mostly empty space explains why most alpha particles in Rutherford's experiment passed through the gold foil undeflected. It revolutionized our understanding of matter, showing that solid objects are not as "solid" as they appear at the atomic level.

8. How did Rutherford's model account for the positive charge in an atom?

Rutherford's model proposed that the positive charge of an atom is concentrated in the small, dense nucleus at the center. This explained the strong repulsion experienced by some alpha particles in his gold foil experiment.

9. How did Rutherford's model contribute to our understanding of atomic mass?

Rutherford's model showed that most of an atom's mass is concentrated in the nucleus. This explained why atoms are so light and mostly empty space, yet materials composed of atoms can be very dense.

10. How did Rutherford's model challenge the indivisibility of atoms?

Rutherford's model showed that atoms have internal structure – a nucleus surrounded by electrons – rather than being indivisible particles. This contradicted the long-held belief in the atom as the smallest, indivisible unit of matter.

11. Why was the large deflection of some alpha particles in Rutherford's experiment so significant?

The large deflection was significant because it indicated the presence of a small, dense, positively charged region (the nucleus) that could repel the positively charged alpha particles. This observation contradicted the prevailing Thomson model and led to a new understanding of atomic structure.

12. What evidence from Rutherford's experiment supported the idea of a nuclear atom?

The key evidence was the observation of a small fraction of alpha particles being deflected at large angles or even backwards. This suggested the presence of a small, dense region of positive charge (the nucleus) capable of strongly repelling the positively charged alpha particles.

13. What role did the concept of "cross-section" play in Rutherford's experiment?

The cross-section in Rutherford's experiment refers to the effective area of the nucleus that could cause significant deflection of alpha particles. The small number of large-angle deflections indicated that this cross-section was very small compared to the atom's total size, leading to the concept of a compact nucleus.

14. What assumptions did Rutherford make in interpreting his gold foil experiment results?

Rutherford assumed that alpha particles were positively charged and much smaller than atoms. He also assumed that the deflections were caused by electrostatic repulsion and that a single deflection event was responsible for large-angle scattering.

15. What is the "Rutherford scattering formula," and what does it describe?

The Rutherford scattering formula mathematically describes the relationship between the angle of deflection of alpha particles and their frequency of occurrence in the gold foil experiment. It supports the nuclear model by showing how the scattering pattern depends on nuclear charge and size.

16. What was Rutherford's gold foil experiment, and how did it lead to his model of the atom?

Rutherford's gold foil experiment involved firing alpha particles at a thin gold foil. Most particles passed through, but some were deflected at large angles. This unexpected result led Rutherford to propose that atoms have a small, dense, positively charged nucleus surrounded by mostly empty space where electrons orbit.

17. What is meant by the "nuclear model" of the atom?

The nuclear model refers to Rutherford's concept that an atom consists of a small, dense, positively charged nucleus surrounded by electrons in mostly empty space. This model emphasizes the concentration of an atom's mass and positive charge in the nucleus.

18. Why was Rutherford's model sometimes called the "planetary model" of the atom?

Rutherford's model was called the planetary model because it depicted electrons orbiting the nucleus like planets around the sun. This analogy helped visualize the structure but also led to some misconceptions about electron behavior.

19. What was the significance of the "Geiger-Marsden experiment" in relation to Rutherford's model?

The Geiger-Marsden experiment, which is another name for Rutherford's gold foil experiment, provided the experimental evidence that led to the nuclear model of the atom. It was crucial in disproving Thomson's plum pudding model and establishing the concept of a nuclear atom.

20. How did Rutherford's model explain the difference in atomic number and mass number?

Rutherford's model suggested that the atomic number is related to the positive charge in the nucleus (later identified as the number of protons), while the mass number is due to the total mass of the nucleus. This laid the groundwork for understanding isotopes.

21. How did Rutherford's model explain the stability of atoms?

Rutherford's model struggled to explain atomic stability. It proposed that electrons orbit the nucleus like planets around the sun, but classical physics predicted that these orbiting electrons should lose energy and spiral into the nucleus, causing atoms to collapse. This limitation led to further developments in atomic theory.

22. What was the major limitation of Rutherford's model regarding electron behavior?

The major limitation was its inability to explain why electrons don't spiral into the nucleus. According to classical physics, orbiting electrons should continuously emit energy and eventually collapse into the nucleus, but this doesn't happen in reality.

23. Why couldn't Rutherford's model explain the emission spectrum of hydrogen?

Rutherford's model didn't account for the discrete emission spectrum of hydrogen because it didn't restrict electrons to specific energy levels. The model allowed for continuous electron orbits, which would produce a continuous spectrum rather than the observed discrete lines.

24. How did Rutherford's model address the issue of electron arrangement around the nucleus?

Rutherford proposed that electrons orbit the nucleus in a manner similar to planets orbiting the sun. However, this model didn't specify the exact arrangement or energy levels of electrons, which was a limitation addressed by later atomic models.

25. How did Rutherford's model contribute to the discovery of the neutron?

Rutherford's model revealed a discrepancy between an element's atomic number and its atomic mass, suggesting the presence of neutral particles in the nucleus. This led to the prediction and subsequent discovery of neutrons by James Chadwick in 1932.

26. What is meant by the "Rutherford atomic number"?

The Rutherford atomic number refers to the number of protons in an atom's nucleus, which Rutherford's work helped to define. This concept became fundamental in understanding elemental identity and the organization of the periodic table.

27. How did Rutherford's model contribute to the understanding of chemical bonding?

While Rutherford's model didn't directly explain chemical bonding, it laid the groundwork by establishing that electrons exist in the space around the nucleus. This led to later models that explained how electrons participate in bonding between atoms.

28. How did Rutherford's model challenge the concept of indivisible atoms proposed by Dalton?

Rutherford's model showed that atoms have internal structure and are not indivisible as Dalton had proposed. By demonstrating the existence of a nucleus and orbiting electrons, Rutherford proved that atoms could be further divided into subatomic particles.

29. What was the significance of the alpha particle choice in Rutherford's experiment?

Alpha particles were ideal for the experiment because they are relatively massive, positively charged, and energetic. Their size and charge made them suitable for probing atomic structure, while their energy allowed them to penetrate the electron cloud and interact with the nucleus.

30. How did Rutherford's model explain the difference between chemical and nuclear reactions?

Rutherford's model suggested that chemical reactions involve interactions between the outer electrons of atoms, while nuclear reactions involve changes in the nucleus itself. This distinction helped explain why nuclear reactions release much more energy than chemical reactions.

31. How did Rutherford's model explain radioactive decay?

Rutherford's model suggested that radioactive decay occurs in the nucleus, explaining why it's unaffected by an atom's chemical environment. This helped separate nuclear phenomena from chemical reactions and led to the field of nuclear physics.

32. What role did probability play in Rutherford's interpretation of his experimental results?

Probability was crucial in Rutherford's interpretation. The small probability of large-angle deflections corresponded to the small size of the nucleus relative to the atom. This probabilistic approach was a precursor to the quantum mechanical view of atomic structure.

33. How did Rutherford's model contribute to the understanding of isotopes?

Rutherford's model suggested that atomic mass is concentrated in the nucleus, while chemical properties are determined by electrons. This laid the groundwork for understanding isotopes as atoms with the same number of protons but different numbers of neutrons.

34. What was the "Rutherford backscattering" phenomenon, and what did it reveal?

Rutherford backscattering refers to the observation that some alpha particles were deflected backwards in the gold foil experiment. This revealed the existence of a small, dense, positively charged nucleus capable of repelling alpha particles strongly enough to reverse their direction.

35. How did Rutherford's model address the issue of atomic size?

Rutherford's model suggested that atoms are mostly empty space with a tiny, dense nucleus. This explained why atoms are much larger than their nuclei and why materials can be compressed – the empty space between nuclei can be reduced.

36. How did Rutherford's model explain the penetrating power of different types of radiation?

Rutherford's model helped explain why alpha particles (helium nuclei) are less penetrating than beta particles (electrons) or gamma rays. The large, positively charged alpha particles interact more strongly with the electrons and nuclei of other atoms, while the smaller beta particles and neutral gamma rays can penetrate further.

37. How did Rutherford's model influence the development of quantum mechanics?

Rutherford's model highlighted the need for a new understanding of electron behavior that didn't follow classical physics. This limitation spurred the development of quantum mechanics to explain atomic structure and electron energy levels.

38. What was the "Rutherford cross-section," and how was it calculated?

The Rutherford cross-section is a measure of the probability of particle scattering at various angles. It was calculated using the scattering formula Rutherford derived, which related the scattering angle to the charge of the nucleus and the energy of the incident particle.

39. What was the role of Ernest Marsden in the development of Rutherford's atomic model?

Ernest Marsden was a student who worked with Rutherford and helped conduct the gold foil experiment. His careful observations, particularly of the rare large-angle scattering events, were crucial in leading to the nuclear model of the atom.

40. What was the significance of the thin gold foil in Rutherford's experiment?

The thin gold foil was crucial because it was only a few atoms thick. This minimized multiple scattering events and allowed Rutherford to observe the effect of single collisions between alpha particles and gold atoms, leading to clearer results.

41. How did Rutherford's model contribute to the development of the Bohr model of the atom?

Rutherford's nuclear model provided the foundation for Bohr's model. Bohr addressed the stability issue in Rutherford's model by proposing quantized electron orbits, combining the nuclear concept with early quantum theory.

42. What was the "Rutherford factor" in atomic scattering experiments?

The Rutherford factor is a term in the scattering formula that describes how the probability of scattering depends on the angle of deflection. It shows that small-angle scattering is much more probable than large-angle scattering, consistent with a small, dense nucleus.

43. How did Rutherford's model explain the neutral charge of atoms?

Rutherford's model proposed that the positive charge in the nucleus is balanced by an equal number of negatively charged electrons orbiting around it. This explained how atoms could be electrically neutral despite containing charged particles.

44. What was the significance of the "Rutherford scattering angle" in his experiment?

The Rutherford scattering angle refers to the degree of deflection of alpha particles in the gold foil experiment. The distribution of these angles provided crucial information about the size and charge of the atomic nucleus.

45. How did Rutherford's model contribute to the understanding of atomic number and atomic mass?

Rutherford's model led to the understanding that the atomic number is related to the nuclear charge (later identified as the number of protons), while the atomic mass is primarily due to the mass of the nucleus. This helped explain the periodic table's structure and the existence of isotopes.

46. What was the "Rutherford-Bohr model," and how did it improve upon Rutherford's original model?

The Rutherford-Bohr model combined Rutherford's nuclear atom with Bohr's concept of quantized electron orbits. It addressed the stability issue in Rutherford's model by proposing that electrons could only exist in specific energy levels, explaining atomic spectra and stability.

47. How did Rutherford's model contribute to the discovery of artificial transmutation?

Rutherford's understanding of the nuclear structure of atoms led him to perform experiments bombarding light elements with alpha particles. This resulted in the first artificial transmutation of elements, converting nitrogen to oxygen, and opened the field of nuclear physics.

48. What was the "Rutherford-Geiger counter," and how was it used in atomic research?

The Rutherford-Geiger counter, developed by Rutherford and Hans Geiger, was an early radiation detector. It was crucial in counting individual alpha particles in scattering experiments, allowing for precise measurements that supported the nuclear model of the atom.

49. How did Rutherford's model explain the concept of atomic radius?

Rutherford's model suggested that atomic radius is primarily determined by the volume of space in which electrons orbit the nucleus. This explained why atomic radii are much larger than nuclear radii and why they vary across the periodic table.

50. What was the "Rutherford scattering cross-section," and how was it measured?

The Rutherford scattering cross-section is a measure of the probability of particle scattering at various angles. It was measured by counting the number of scattered particles at different angles and comparing these to the predictions of Rutherford's scattering formula.

51. How did Rutherford's model contribute to the understanding of nuclear forces?

Rutherford's model revealed the need for a new force to explain why positively charged protons could coexist in the nucleus despite electrostatic repulsion. This led to the discovery of the strong nuclear force, which overcomes electromagnetic repulsion at short distances.

52. What was the significance of the "Rutherford-Soddy theory of radioactive decay"?

The Rutherford-Soddy theory explained radioactive decay as a spontaneous process occurring within the atomic nucleus. It introduced the concept of half-life and showed that radioactive decay could transform one element into another, leading to the understanding of radioactive series.

53. How did Rutherford's model influence the development of nuclear energy and weapons?

Rutherford's model provided the foundation for understanding nuclear structure and reactions. This knowledge was crucial in the development of nuclear fission and fusion processes, leading to both nuclear energy production and the creation of nuclear weapons.

54. What was the "Rutherford-Bohr atom," and how did it address spectral lines?

The Rutherford-Bohr atom combined Rutherford's nuclear model with Bohr's quantized orbits. It explained spectral lines by proposing that electrons could only transition between specific energy levels, emitting or absorbing photons of specific frequencies in the process.

55. How did Rutherford's model contribute to the modern understanding of electron configuration?

While Rutherford's model didn't directly address electron configuration, it established the concept of electrons orbiting a nucleus. This laid the groundwork for later models that explained electron shells, subshells, and orbitals, leading to our modern understanding of electron configuration and chemical behavior.